Reactivity 3.2 Electron transfer reactions (HL)

Reactivity 3.2.12

Understandings:

Understandings:

**The hydrogen half-cell H2(g)**⇌**2H****+****(aq) + 2e****–****is assigned a standard electrode potential of zero by convention. It is used in the measurement of standard electrode potential,**⦵.*E*

- Interpret standard electrode potential data in terms of ease of oxidation/reduction.

- Standard electrode potentials are given in the data booklet.

Reactivity 3.2.13

Understandings:

Understandings:

**Standard cell potential,**⦵*E***, can be calculated from standard potentials.**⦵*E***has a positive value for a spontaneous**

- Predict whether a reaction is spontaneous in the forward or reverse direction from
*E*⦵.

Reactivity 3.2.14

Understandings:

Understandings:

**The equation****Δ**⦵*G***= −**⦵*nFE***shows the relationship between standard****cell****change in Gibbs energy and standard electrode potential for a reaction.**

- Determine the value for Δ
*G*⦵ from*E*⦵ data.

- The equation and the value of
*F*in C mol–1 are given in the data booklet.

- Reactivity 1.4 How can thermodynamic data also be used to predict the spontaneity of a reaction?

Reactivity 3.2.15

Understandings:

Understandings:

**During electrolysis of aqueous solutions, competing reactions can occur at the anode and cathode, including the oxidation and reduction of water.**

- Deduce from standard electrode potentials the products of the electrolysis of aqueous solutions.

- Electrolytic processes should include the electrolysis of water and of aqueous solutions.

Reactivity 3.2.16

Understandings:

Understandings:

**Electroplating involves the electrolytic coating of an object with a metallic thin layer.**

- Deduce equations for the electrode reactions during electroplating.